16.1 Introduction to Acids and Bases

[@rayx4703]

If this man was my professor right now, I would be able to become a chem prof myself

[@ChadsPrep]

Excellent!

[@zeekstersthename8014]

outstanding! I understood every single thing. Literally man! keep coming out with more, please!

[@ChadsPrep]

That's the plan Zakaria! Glad you're finding my videos helpful!

[@juliannenelson7309]

Where have you been all my chemistry life!

[@ChadsPrep]

Great question, Julianne - glad you found us! Happy Studying!

[@ambercorueil1114]

These videos are saving my grade!! You are so good at teaching

[@BUNNYnotFUNNY]

I have to thank you so much. I have a horrible chemistry professor and I have to come watch your videos to understand fully. Thank you so much you are amazing at teaching

[@ChadsPrep]

You're very welcome Nyah! Glad you're finding my lessons helpful!

[@joeburreaux7953]

Hey Chad, while your videos are great, I highly recommend you update this Chemistry course when you have the time, as it has been nearly 4 years! Not that much has changed, but I really like how different your new Orgo series looked from the 2018 version. I think this course could be fine tuned a little bit with a better camera and newer practice problems. Thanks!

[@ChadsPrep]

Hello Joe and thanks for the feedback! I completely agree which is why I'll be remaking and posting the entire series throughout the next school year. You should begin seeing new Gen Chem videos in the second half of August! Happy Studying!

[@halicusdiaarcan102]

Whoa just 17 minutes and a quick response! That's the fastest I've seen a youtuber respond to a comment in an older video :O

[@ChadsPrep]

And just 10 hours to respond to yours :( Hello Halicus! Sometimes I'm in a position to be more prompt than others, but I try! Happy Studying!

[@christophergalin4795]

Water does have a polyatomic ion in it though. Isnt it OH- technically? (Referring back to when you are talking about Binary Acids. (Oxyacids) Would water be considered an Oxyacid too?

[@thatbossguy123]

Hi Chad, I just want to make sure that we can also explain acidity periodic table trend with the following thoughts: As you go across from left to right on the periodic table, the Zeff charge increases and a more positive Zeff charge can stabilize the negative charge of the conjugate base better, making the CB more stable which in turn increases the acidity of the conjugate acid. Is this the same thing that EN rule basically says? What is the explanation behind more EN atoms can better stabilize the CB and therefore yield a stronger acid? Also can you think about going down the periodic table means the size of the atom of the conjugate base increases and so the negatively charged CB can better stabilize its negative charge with a larger atom, leading to a more stable CB and therefore a stronger conjugate acid? And also for oxyacids, the more Os, the stronger the acid because the CB will be resonance stabilized but would inductive effect play a role in also stabilizing the negative CB? Also for the oxyacid rule that more EN heteroatom will be more acidic, is that based off the inductive effect of EN atoms? Thank you so much!

[@thatbossguy123]

Oh I understand why EN atoms can better stabilize the CB now.

[@ChadsPrep]

@@thatbossguy123 Awesome! While Zeff, size, and electronegativity are all related, a discussion of acidity is usually only explained in terms of size (for atoms in the same group) or electronegativity (for atoms in the same period) and leaves Zeff out of the discussion entirely. Hope this helps!

[@thatbossguy123]

@@ChadsPrep Gotcha, thanks! I also had a couple more questions that do not appear unless you click "show more." It would be really awesome if you could address those questions I have but if not I understand. As always thanks for the awesome videos and quick response! -Greg

[@ChadsPrep]

@@thatbossguy123 You have more questions associated with this video? I don't see them at all. You can also email me at [e-mail]

[@thatbossguy123]

@@ChadsPrep I emailed you! Thanks so much!

[@deborahaigbedion6323]

hello i know you mentioned that HF is a weak acid but wouldn't it also be considered as a strong acid due to it being electronegativley strong ??

[@ChadsPrep]

Not in this case Deborah. The distinction between strong and weak is simply whether or not it dissociates 'completely' in water. HF is definitely a weak acid under this definition. It's Ka is 6.8x10^-4. The Ka values for all of the strong acids are considerably larger than 1. Hope this helps!

[@thatbossguy123]

Hey chad! Quick question: For the oxoacids, do more oxygens also translate into making Cl more partially positively charged and better able to stabilize the negative charge on the oxygen? And in regards to the fact that more EN heteroatom is more acidic, can you also view this in terms of inductive effect or that a more EN atom will be better able to spread out the negative charge on the oxygen better? Thanks!

[@ChadsPrep]

Oxoacids with the same central atom but more oxygens are more acidic predominantly due to the additional resonance-stabilization of the conjugate base. If you try to make an argument for the inductive effect you end up with a chicken and egg problem. If the central atom is bonded to more electronegative oxygen atoms then the oxygen atoms will steal more electron density away from the central atom making it more positive. But now we would try to say that because the central atom is more positive then it could steal more electron density away from the oxygen atoms??? There is a subtle sense in which we might try to craft an argument along these lines but I've never seen it discussed anywhere and it would be very, very minor in comparison to resonance regardless. Hope this helps!

[@curtpiazza1688]

Great review.....thanx!

[@ChadsPrep]

Glad to hear it, Curt!

[@obaapapapabi3015]

Great

[@ChadsPrep]

Glad to hear it!

[@Manoamanoamano]

Chad can you please write my DAT for me? Thanks

[@admissionuniversity5753]

nice teaching sir please use good resolution camera as result i can see it

[@ChadsPrep]

👍

[@calliopeberenices3851]

I've always hated chemistry and was crazy over physics only! Until I've come across this video. Thank you so much Sir for this fantastic break down on acids and bases. Keep making videos. I subscribed 😁👍

[@ChadsPrep]

Glad you found us, Calliope - Thanks for subscribing!

[@farmerfromwisconsin7256]

At 16:35 , How can HI be stronger than HBr, Don't they both ionize 100%?

[@ChadsPrep]

You're exactly right, they do both ionize in water. In fact all the strong acids do and therefore the strongest acid present in any aqueous solution of any strong acid is H3O+. Therefore they all appear equally strong in water which we call the 'leveling effect.' However, change the solvent from water to something else in which they don't all dissociate completely and we can begin to tell them apart, and we do indeed find that HI is a stronger acid than HBr. Hope this helps!

[@farmerfromwisconsin7256]

@@ChadsPrep I love you sir, Thank you so much

[@farmerfromwisconsin7256]

How do we know if a compound can accept an H+. Anything can accept H+, right? (Weird stuff like NH3, etc.) So does that mean every compound is a base? Thanks again

[@ChadsPrep]

The most fundamental requirement is that you need an atom with a lone pair of electrons. 😀